Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

What is the energy difference between the two lowest energy levels for a proton in a cubical box with side length 1.00 \(\times\) 10\(^{-14}\) m, the approximate diameter of a nucleus?

Short Answer

Expert verified
The energy difference \(\Delta E = 2.42 \times 10^{-13}\) J.

Step by step solution

01

Understand the system

The problem involves a proton confined in a cubical box, a situation where quantum mechanics is applicable. We will use the particle in a box model to calculate energy levels.
02

Know the Energy Formula for a Cubical Box

The energy levels for a particle in a 3D box are given by\[E_{n_x, n_y, n_z} = \frac{h^2}{8mL^2} (n_x^2 + n_y^2 + n_z^2)\]where \(h\) is Planck's constant, \(m\) is the mass of the proton, \(L\) is the side of the box, and \(n_x, n_y, n_z\) are quantum numbers (1, 2, 3,...).
03

Set Quantum Numbers for Two Lowest Energy Levels

The lowest energy state is the ground state with \(n_x = n_y = n_z = 1\). The next energy state involves exciting one quantum number by an integer; often it's \(n_x = 2, n_y = n_z = 1\).
04

Calculate Ground State Energy

For the ground state, where \(n_x = n_y = n_z = 1\), the energy is:\[E_{1,1,1} = \frac{h^2}{8mL^2}(1^2 + 1^2 + 1^2) = \frac{3h^2}{8mL^2}\]
05

Calculate First Excited State Energy

For the first excited state, a potential scenario is \(n_x = 2, n_y = n_z = 1\), giving:\[E_{2,1,1} = \frac{h^2}{8mL^2}(2^2 + 1^2 + 1^2) = \frac{6h^2}{8mL^2}\]
06

Compute Energy Difference

The energy difference between the first excited state and the ground state is:\[\Delta E = E_{2,1,1} - E_{1,1,1} = \left(\frac{6h^2}{8mL^2}\right) - \left(\frac{3h^2}{8mL^2}\right) = \frac{3h^2}{8mL^2}\]
07

Insert Values to Find Numerical Result

Insert the values for Planck's constant \(h = 6.626 \times 10^{-34}\, \text{Js}\), the mass of the proton \(m = 1.673 \times 10^{-27}\, \text{kg}\), and the side length \(L = 1.00 \times 10^{-14}\, \text{m}\):\[\Delta E = \frac{3 \times (6.626 \times 10^{-34})^2}{8 \times 1.673 \times 10^{-27} \times (1.00 \times 10^{-14})^2}\]
08

Calculate Final Numerical Solution

Carry out the computation in step 7 to find \(\Delta E\).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Particle in a Box
The "particle in a box" is a popular model in quantum mechanics. It simplifies the complex nature of particles confined in a limited space, like the nucleus of an atom. Think of it as a way to visualize how particles behave when trapped in a very tiny space.

In this model, the box is usually considered to have infinitely high walls, meaning the particle cannot escape. It's a useful concept because it allows us to calculate the possible energy levels of the particle based on their quantized nature. In our specific problem, a proton is considered to be in such a box, which represents the confined space of a nucleus. The cubical shape we use is idealized to make the math easier, but it captures the essential physics.
Energy Levels
Energy levels in quantum mechanics are like "rungs on a ladder." A particle can only exist on these specific steps and nowhere in between.

When we talk about energy levels in the "particle in a box" model, these levels are determined numerically using an equation. This equation includes quantum numbers, Planck's constant, the mass of the particle, and the size of the confinement region (like our cubical box). Different arrangements of quantum numbers create different energy levels.
  • The ground state is the lowest energy level, where the quantum numbers are all minimized (e.g., 1, 1, 1).
  • Excited states are higher energy levels where at least one quantum number is increased.
This is how we derive energy levels for our proton in the box.
Planck's Constant
Planck's constant is a fundamental constant in physics that plays an essential role in quantum mechanics. It defines the size of the quantization found in nature.

In the formula for the "particle in a box," Planck's constant appears as a squared value. This constant, denoted as \( h \), is incredibly small, approximately \( 6.626 \times 10^{-34} \text{Js} \). Its tiny size indicates that the energy differences we're discussing are extremely small at the quantum level.

Planck's constant essentially "scales" the quantum mechanical world to its microscopic nature, affecting how we calculate energy levels and the precise nature of quantum jumps between these levels.
Quantum Numbers
Quantum numbers are key to understanding the quantized nature of particles in quantum mechanics. In the "particle in a box" model, they help define the possible energy levels.

There are typically three quantum numbers \( n_x \), \( n_y \), and \( n_z \) in a three-dimensional box. Each of these numbers can be an integer starting from 1.
  • The smallest numbers represent the lowest energy state, or ground state.
  • Higher numbers indicate excited states.
These values are crucial for calculating the energy levels using the formula provided. By changing these numbers, you compute different energy scenarios for the particle, such as moving from ground state to an excited state, which is what causes energy differences as per our calculations.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

For germanium (\(Ge, Z = 32\)), make a list of the number of electrons in each subshell (\(1s, 2s, 2p,\dots\)). Use the allowed values of the quantum numbers along with the exclusion principle; do not refer to Table 41.3.

A hydrogen atom undergoes a transition from a 2\(p\) state to the 1\(s\) ground state. In the absence of a magnetic field, the energy of the photon emitted is 122 nm. The atom is then placed in a strong magnetic field in the z-direction. Ignore spin effects; consider only the interaction of the magnetic field with the atom's orbital magnetic moment. (a) How many different photon wavelengths are observed for the 2p \(\rightarrow\) 1s transition? What are the \(m$$_l\) values for the initial and final states for the transition that leads to each photon wavelength? (b) One observed wavelength is exactly the same with the magnetic field as without. What are the initial and final \(m$$_l\) values for the transition that produces a photon of this wavelength? (c) One observed wavelength with the field is longer than the wavelength without the field. What are the initial and final \(m$$_l\) values for the transition that produces a photon of this wavelength? (d) Repeat part (c) for the wavelength that is shorter than the wavelength in the absence of the field.

(a) The doubly charged ion \(N^{2+}\) is formed by removing two electrons from a nitrogen atom. What is the ground-state electron configuration for the \(N^{2+}\) ion? (b) Estimate the energy of the least strongly bound level in the \(L\) shell of \(N^{2+}\). (c) The doubly charged ion \(P^{2+}\) is formed by removing two electrons from a phosphorus atom. What is the ground-state electron configuration for the \(P^{2+}\) ion? (d) Estimate the energy of the least strongly bound level in the \(M\) shell of \(P^{2+}\).

Assume that the researchers place an atom in a state with \(n\) = 100, \(l\) = 2. What is the magnitude of the orbital angular momentum \(L\) associated with this state? (a) \(\sqrt{2} \space\hslash \); (b) \(\sqrt{6} \space\hslash\); (c) \(\sqrt{200}\space \hslash\); (d) \(\sqrt{10,100}\space \hslash \).

(a) Make a chart showing all possible sets of quantum numbers \(l\) and \(m$$_l\) for the states of the electron in the hydrogen atom when n = 4. How many combinations are there? (b) What are the energies of these states?

See all solutions

Recommended explanations on Physics Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free